Draw the Lewis structure for methane, CH4. EXERCISE! Draw the Lewis structure for methane, CH4. What is the shape of a methane molecule? What are the bond angles? The shape of CH4 is tetrahedral. The bond angles are 109.5o. Copyright © Cengage Learning. All rights reserved

What is the valence electron configuration of a carbon atom? CONCEPT CHECK! What is the valence electron configuration of a carbon atom? Why can’t the bonding orbitals for methane be formed by an overlap of atomic orbitals? The valence electron configuration of a carbon atom is s2p2. Because this would lead to two different types of C-H bonds and we know that methane has four identical C-H bonds that are 109.5° apart from each other (not 90° from each other). Copyright © Cengage Learning. All rights reserved

Bonding in Methane Assume that the carbon atom has four equivalent atomic orbitals, arranged tetrahedrally. Copyright © Cengage Learning. All rights reserved

Hybridization Mixing of the native atomic orbitals to form special orbitals for bonding. Copyright © Cengage Learning. All rights reserved

sp3 Hybridization Combination of one s and three p orbitals. Whenever a set of equivalent tetrahedral atomic orbitals is required by an atom, the localized electron model assumes that the atom adopts a set of sp3 orbitals; the atom becomes sp3 hybridized. The four orbitals are identical in shape. Copyright © Cengage Learning. All rights reserved

An Energy-Level Diagram Showing the Formation of Four sp3 Orbitals Copyright © Cengage Learning. All rights reserved

The Formation of sp3 Hybrid Orbitals Copyright © Cengage Learning. All rights reserved

Tetrahedral Set of Four sp3 Orbitals Copyright © Cengage Learning. All rights reserved

Draw the Lewis structure for C2H4 (ethylene)? EXERCISE! Draw the Lewis structure for C2H4 (ethylene)? What is the shape of an ethylene molecule? What are the approximate bond angles around the carbon atoms? The shape of an ethylene molecule is trigonal planar around each carbon atom. The approximate angles are 120o. Copyright © Cengage Learning. All rights reserved

Why can’t sp3 hybridization account for the ethylene molecule? CONCEPT CHECK! Why can’t sp3 hybridization account for the ethylene molecule? Because sp3 hybrid orbitals are at angles of 109.5o rather than the required 120o. Copyright © Cengage Learning. All rights reserved

sp2 Hybridization Combination of one s and two p orbitals. Gives a trigonal planar arrangement of atomic orbitals. One p orbital is not used. Oriented perpendicular to the plane of the sp2 orbitals. Copyright © Cengage Learning. All rights reserved

Sigma (Σ) Bond Electron pair is shared in an area centered on a line running between the atoms. Copyright © Cengage Learning. All rights reserved

Pi (Π) Bond Forms double and triple bonds by sharing electron pair(s) in the space above and below the σ bond. Uses the unhybridized p orbitals. Copyright © Cengage Learning. All rights reserved

An Orbital Energy-Level Diagram for sp2 Hybridization Copyright © Cengage Learning. All rights reserved

The Hybridization of the s, px, and py Atomic Orbitals Copyright © Cengage Learning. All rights reserved

Formation of C=C Double Bond in Ethylene To play movie you must be in Slide Show Mode PC Users: Please wait for content to load, then click to play Mac Users: CLICK HERE Copyright © Cengage Learning. All rights reserved

Draw the Lewis structure for CO2. EXERCISE! Draw the Lewis structure for CO2.  What is the shape of a carbon dioxide molecule? What are the bond angles? The shape of CO2 is linear. The bond angles are 180o. Copyright © Cengage Learning. All rights reserved

sp Hybridization Combination of one s and one p orbital. Gives a linear arrangement of atomic orbitals. Two p orbitals are not used. Needed to form the π bonds. Copyright © Cengage Learning. All rights reserved

The Orbital Energy-Level Diagram for the Formation of sp Hybrid Orbitals on Carbon Copyright © Cengage Learning. All rights reserved

When One s Orbital and One p Orbital are Hybridized, a Set of Two sp Orbitals Oriented at 180 Degrees Results Copyright © Cengage Learning. All rights reserved

The Orbitals for CO2 Copyright © Cengage Learning. All rights reserved

Draw the Lewis structure for PCl5. EXERCISE! Draw the Lewis structure for PCl5. What is the shape of a phosphorus pentachloride molecule? What are the bond angles? The shape is trigonal bipyramidal with bond angles of 90o and 120o. Copyright © Cengage Learning. All rights reserved

dsp3 Hybridization Combination of one d, one s, and three p orbitals. Gives a trigonal bipyramidal arrangement of five equivalent hybrid orbitals. Copyright © Cengage Learning. All rights reserved

The Orbitals Used to Form the Bonds in PCl5 Copyright © Cengage Learning. All rights reserved

Draw the Lewis structure for XeF4. EXERCISE! Draw the Lewis structure for XeF4. What is the shape of a xenon tetrafluoride molecule? What are the bond angles? The shape is octahedral with bond angles of 90o and 180o. Copyright © Cengage Learning. All rights reserved

d2sp3 Hybridization Combination of two d, one s, and three p orbitals. Gives an octahedral arrangement of six equivalent hybrid orbitals. Copyright © Cengage Learning. All rights reserved

How is the Xenon Atom in XeF4 Hybridized? Copyright © Cengage Learning. All rights reserved

Draw the Lewis structure for HCN. Which hybrid orbitals are used? CONCEPT CHECK! Draw the Lewis structure for HCN. Which hybrid orbitals are used? Draw HCN: Showing all bonds between atoms. Labeling each bond as σ or π. sp hybrid orbitals are used in the bonding of HCN. Two sigma bonds and two pi bonds are present. Copyright © Cengage Learning. All rights reserved

CONCEPT CHECK! Determine the bond angle and expected hybridization of the central atom for each of the following molecules: NH3 SO2 KrF2 CO2 ICl5 NH3 – 109.5o, sp3 SO2 – 120o, sp2 KrF2 – 90o, 120o, dsp3 CO2 – 180o, sp ICl5 – 90o, 180o, d2sp3